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1. Use the ideal gas law to determine the number of moles of carbon dioxide gas in the flask. For the pressure, use AP.

1. Use the ideal gas law to determine the number of moles of carbon dioxide gas in the flask. For the pressure, use AP.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please please with the data table provide please do the calculations in the image attached
Mass of a whole tablet: 3.2338g Mass of portion of tablet used Volume of flask Initial Pressure Maximum Pressure ΔΡ Temperature Trial 1 2.0839 138.5 mL 105.89 KPa 126.92 K Pa 21.03 18.4°C Trial 2 2.0549 138.5mL 104.81 KPa [25.27 кра 20.46 18.3°C Trial 3 2.061g 138.5 mL 105.23 KPa 125.54 k Pa 20.31 18.3°C
Transcribed Image Text:Mass of a whole tablet: 3.2338g Mass of portion of tablet used Volume of flask Initial Pressure Maximum Pressure ΔΡ Temperature Trial 1 2.0839 138.5 mL 105.89 KPa 126.92 K Pa 21.03 18.4°C Trial 2 2.0549 138.5mL 104.81 KPa [25.27 кра 20.46 18.3°C Trial 3 2.061g 138.5 mL 105.23 KPa 125.54 k Pa 20.31 18.3°C
CALCULATIONS (Show one sample calculation in your lab notebook; ie, one trial) 1. Use the ideal gas law to determine the number of moles of carbon dioxide gas in the flask. For the pressure, use AP. 2. Now take the number of moles of CO₂ calculated in (1) and add to it the moles of 8.5mg of CO₂ per 5mL of acid solution, which is assumed to be dissolved in the solution. This is the total amount of carbon dioxide produced (per trial). 3. Use your result in (2) and the stoichiometry of the balanced equation to find the mass of NaHCO3. g NaHCO3: (Triall) (Trial 2) (Trial 3) 4. Use the results from (3) and the mass of the portion of tablet used to calculate the mass percentage of NaHCO3 in your Alka-Seltzer preparation. Also give the average and the relative range. % NaHCO3: Average: (Trial1) (Trial 2) Relative Range: (Trial 3) 5. Calculate the mass percentage of sodium bicarbonate from the mass claimed on the label. % NaHCO3 6. Taking the label as the true value, calculate the relative error of your average % NaHCO3. % error
Transcribed Image Text:CALCULATIONS (Show one sample calculation in your lab notebook; ie, one trial) 1. Use the ideal gas law to determine the number of moles of carbon dioxide gas in the flask. For the pressure, use AP. 2. Now take the number of moles of CO₂ calculated in (1) and add to it the moles of 8.5mg of CO₂ per 5mL of acid solution, which is assumed to be dissolved in the solution. This is the total amount of carbon dioxide produced (per trial). 3. Use your result in (2) and the stoichiometry of the balanced equation to find the mass of NaHCO3. g NaHCO3: (Triall) (Trial 2) (Trial 3) 4. Use the results from (3) and the mass of the portion of tablet used to calculate the mass percentage of NaHCO3 in your Alka-Seltzer preparation. Also give the average and the relative range. % NaHCO3: Average: (Trial1) (Trial 2) Relative Range: (Trial 3) 5. Calculate the mass percentage of sodium bicarbonate from the mass claimed on the label. % NaHCO3 6. Taking the label as the true value, calculate the relative error of your average % NaHCO3. % error
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